Using Le Chatilier's Pronciple to predict whether adding some HClO (aq) causes the system to shift in the direction to products or reactions: HClO + H20= H20+ ClO

The rate of decomposition of SO, Cl2 according to the reaction so,Cl, (s) → SO2(g) + Cl2 (g) can be followed by monitoring the total pressure in the reaction vessel. Consider the following data. Time (s) Total Pressure (torr) 491.7 180.9 548.7 434.0 618.4 605.7 659.1 916.7 721.7 1233.3 773.0 1504.9 809.0 2015.2 860.7 Convert these total pressures into changes in the pressure of the SO, Cl, manipulate the data as needed, and then use a graphing calculator or spreadsheet to plot the data to determine the order of the reaction and the rate constant. What is the order of the reaction? O zero-order O frst-order O second-order Determine the value and unit of the rate constant. (Enter an unrounded value.) k =

Consider the following reaction: 4PC13(g) P4(g) + 6C12(g) If the initial concentration of PC13(g) is 1.5 mol/L, and "x" is the equilibrium concentration of Pa(g), what is the correct equilibrium relation а. Кс-бх7 O b. Kc=6x7/(1.0-4x)4 O c. Kc=(x)(6x)6/(1.0-4x)4 O d. Kc=(x)(6x)°/(1.5-4x)4 O e. Kc=x'/(1.0-x)4

Using the information provided, determine the enthalpy (in kJ/mol) for the reaction 2 K(s) + 2 H₂O(l) → 2 KOH (aq) + H₂(g) K (s) = 0 kJ/mol H2O(l) = -285.8 kJ/mol KOH(aq) = -482.4 kJ/mol H2(g)= 0 kJ/mol

The reverse copper disproportion reaction has been proposed to etch solid copper: Cu + Cu²¹(1)→ 2Cu* (1) Determine the equilibrium constant of the disproportionation reaction using the following half-cell reactions: Cu²+ (1) + e → Cut (1) Cu Cu (1) + e E = 0.153 V Eº: - 0.521 V ==

I need help finding the rate constant

Solve correctly please. (Will provide helpful ratings for correct solution)